True/false
1. will addding a strong acid (HNO3) to a solution that is 0.010M in Ag(NH3)2(^+) will tend to dissociate the complex ion into Ag+ and NH4+
2.adding a strong acid (HNO3)to a solution that is 0.010M in AgBr2(^-) will tend to dissociate the complex ion into Ag+ and Br-
3.to dissolve AgI, one can add either NaCN or HCN as a source fo the cyanide-complexing ligand. Fewer moles of NaCN would be required.
4. Solution A is 0.10M in Br- and contains the complex ion Ag(Br)2(^-). Solution B is 0.10M in CN- and contains the complex ion Ag(CN)2 (^-). Solution B will have more particles of complex ion per particle of Ag+ than solution A.
1. False. To determine whether adding a strong acid (HNO3) to a solution of Ag(NH3)2(^+) will dissociate the complex ion into Ag+ and NH4+, we need to consider the stability of the complex. In this case, Ag(NH3)2(^+) is a complex ion formed from Ag+ and ammonia ligands (NH3). The complex ion is held together through coordination bonds. HNO3 is a strong acid and can potentially react with the ammonia ligands, but it is unlikely to fully dissociate the complex ion. To confirm this, we need to refer to the stability constant of the complex ion and the equilibrium constant of the reaction.
2. False. Similar to the explanation above, adding a strong acid (HNO3) to a solution of AgBr2(^-) will not directly dissociate the complex ion into Ag+ and Br-. AgBr2(^-) is a complex ion formed from Ag+ and bromide ligands (Br-). The complex ion is held together through coordination bonds. While HNO3 can potentially react with the bromide ligands, it is unlikely to fully dissociate the complex ion. Again, we would need to refer to the stability constant of the complex ion and the equilibrium constant of the reaction to obtain a definitive answer.
3. True. To dissolve AgI, both NaCN and HCN can be used as a source of the cyanide-complexing ligand. The formation of a stable complex with Ag+ will help dissolve AgI. However, since NaCN is a stronger source of cyanide ions than HCN, fewer moles of NaCN would be required. This is because NaCN completely dissociates in water, providing a higher concentration of cyanide ions compared to HCN, which only partially dissociates.
4. True. Solution B, which is 0.10M in CN- and contains the complex ion Ag(CN)2(^-), will have more particles of the complex ion per particle of Ag+ than Solution A, which is 0.10M in Br- and contains the complex ion Ag(Br)2(^-). This is because Ag(CN)2(^-) has a 2:1 stoichiometry, meaning that for every Ag+ ion, there are two CN- ligands present. On the other hand, Ag(Br)2(^-) has a 1:2 stoichiometry, meaning that for every Ag+ ion, there are two Br- ligands present. Thus, Solution B will have a higher concentration of complex ions per Ag+ ion compared to Solution A.